The first-order rate constant for the decomposition of CH3N₂CH3, CH3N₂CH3(g) → C₂H5(9) + N₂(g) at 327 °C is k = 3.60e- 04 s ¹. Suppose we start with 0.0858 mol of CH3N₂CH3 in a volume of 6.9 L. How many moles of CH3N₂CH3 will remain after 3.79e+01 min? a) 0.0846 moles will remain. b) 0.00117 moles will remain. c) 6.81e-79 moles will remain. d) 0.0703 moles will remain. e) 0.0378 moles will remain.

The first-order rate constant for the decomposition of CH3N₂CH3, CH3N₂CH3(g) → C₂H5(9) + N₂(g) at 327 °C is k = 3.60e- 04 s ¹. Suppose we start with 0.0858 mol of CH3N₂CH3 in a volume of 6.9 L. How many moles of CH3N₂CH3 will remain after 3.79e+01 min? a) 0.0846 moles will remain. b) 0.00117 moles will remain. c) 6.81e-79 moles will remain. d) 0.0703 moles will remain. e) 0.0378 moles will remain.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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